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Chemistry
Chemistry
Problem
For the decomposition of
N
2
O
(
g
)
\text{N}_2\text{O}(g)
N
2
O
(
g
)
at
700
K
700\,\text{K}
700
K
,
log
10
K
p
=
−
2.35
\log_{10}K_p=-2.35
lo
g
10
K
p
=
−
2.35
when the equation is written as
N
2
O
(
g
)
⇌
N
2
(
g
)
+
1
2
O
2
(
g
)
\text{N}_2\text{O}(g)\rightleftharpoons\text{N}_2(g)+\tfrac12\text{O}_2(g)
N
2
O
(
g
)
⇌
N
2
(
g
)
+
2
1
O
2
(
g
)
. Calculate
log
10
K
p
\log_{10}K_p
lo
g
10
K
p
for the reaction written in the opposite direction at the same temperature.
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